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WorksheetsAQA GCSE CHEMISTRY - QUANTATIVE CHEMISTRY
Total questions: 26
Worksheet time: 13mins
N2 + O2 → 2NO
What mass of nitrogen is needed to make 120 g of nitrogen monoxide (NO)?
(Ar: N = 14, O = 16)
(Higher Tier Question)
30 g
4 g
120 g
56 g
What does the following equation show? Mg + 2HCl → MgCl2 + H2
(Higher Tier Question)
1 mole of magnesium reacts with 1 mole of hydrochloric acid to make 2 moles of magnesium chloride and 1 mole of hydrogen
1 mole of magnesium reacts with 2 moles of hydrochloric acid to make 2 moles of magnesium chloride and 1 mole of hydrogen
1 mole of magnesium reacts with 2 moles of hydrochloric acid to make 1 mole of magnesium chloride and 1 mole of hydrogen
This reaction isn't possible
Iron reacts with oxygen to form iron oxide. Which of these shows the numbers needed to form the correct balanced equation?
AFe + BO2 → CFe2O3
A = 2, B = 3, C = 2
A = 4, B = 3, C = 2
A = 2, B = 6, C = 2
A = 1, B = 1, C = 2
What is the relative formula mass of CO (carbon monoxide)?
(Ar: C = 12, O = 16)
12
16
38
28
What does the law of conservation of mass tell you about the mass of the reactants and the mass of the products in a reaction?
The mass of the reactants is always double the mass of the products
The mass of the reactants is more than the mass of the products
The mass of the products is more than the mass of the reactants
The mass of the products equals the mass of the reactants
How many iron, nitrogen and oxygen atoms are there in Fe(NO3)3?
3 iron atoms, 3 nitrogen atoms and 6 oxygen atoms
3 iron atoms, 3 nitrogen atoms and 9 oxygen atoms
1 iron atom, 1 nitrogen atom and 3 oxygen atoms
1 iron atom, 3 nitrogen atoms and 9 oxygen atoms
How many magnesium, oxygen and hydrogen atoms are there in Mg(OH)2?
1 magnesium atom, 1 oxygen atom and 2 hydrogen atoms
1 magnesium atom, 2 oxygen atoms and 2 hydrogen atoms
2 magnesium atoms, 2 oxygen atoms and 2 hydrogen atoms
1 magnesium atom, 2 oxygen atoms and 1 hydrogen atom
What is the relative formula mass of Fe(NO3)3?
(Ar: Fe = 56, N = 14, O = 16)
118
86
214
242
Which of these statements about the number of atoms in a mole is correct?
(Higher Tier Question)
The number of atoms in a mole of carbon is the same as the number of molecules in a mole of carbon dioxide
The number of atoms in a mole of carbon is half the number of molecules in a mole of carbon dioxide
The number of atoms in a mole of carbon is higher than the number of molecules in a mole of carbon dioxide
The number of atoms in a mole of carbon is smaller than the number of molecules in a mole of carbon dioxide
S + O2 → SO2
What is the maximum mass of sulfur dioxide that can be made from 16 g of sulfur?
(Ar: S = 32, O = 16)
(Higher Tier Question)
32 g
16 g
0.5 g
64 g
The sum of the relative atomic masses of the products in a particular balanced equation is 242.
What is the sum of the relative atomic masses of the reactants?
121
242
243
241
Sodium reacts with chlorine to form sodium chloride.
__Na + Cl2 → 2NaCl
What is the missing number needed to balance the equation?
1
2
3
4
What is the relative formula mass of sodium oxide (Na2O)?
(Ar: Na = 23, O = 16)
62
39
55
46
Calculate the mass of 0.25 mol of carbon dioxide molecules.
(Mr: CO2 = 44)
(Higher Tier Question)
33 g
11 g
12 g
16 g
What does conservation of mass mean?
No atoms are lost or made during a chemical reaction
Some atoms are lost but none are made during a chemical reaction
No atoms are lost but some are made during a chemical reaction
Atoms can be made or lost in a chemical reaction
Which of these will definitely increase the concentration of a solution?
(Higher Tier Question)
Adding more solvent to a solution
Evaporating some of the solvent so the volume of the solution is reduced
Increasing the volume of the solution
Decreasing the volume of the solution
The number of atoms, molecules or ions in a mole of a substance is the Avogadro constant.
What is the value of the Avogadro constant?
Choose the correct power of ten, to complete 6.02 × 10??
(Higher Tier Question)
-13
13
-23
23
In a chemical reaction involving two reactants, it is common to use one of the reactants in excess. Why is this?
(Higher Tier Question)
Because one reactant is always cheaper
Because it ensures the other reactant is completely used up
Because it is easier than using the same amount of each reactant
Because it makes sure both reactants are used up
Calculate the number of moles of water molecules in 36 g of water.
(Mr: H2O = 18)
(Higher Tier Question)
2 mol
0.5 mol
18 mol
16 mol
A solution of sodium chloride has a concentration of 10 g/dm3.
What mass of sodium chloride is dissolved in 2 dm3 of the solution?
10 g
20 g
2 g
5 g
What is the mass of 1 mole of water?
(Higher Tier Question)
16 g
2 g
18 g
6.02 g
The sum of the relative atomic masses of the reactants in a particular balanced equation is 100.
What is the sum of the relative atomic masses of the products?
50
100
1000
99
What is the relative formula mass of Mg(OH)2?
(Ar: Mg = 24, H = 1, O = 16)
41
39
42
58
How many chlorine atoms are there in Cl2?
1
2
3
4
2Mg(s) + O2(g) → 2MgO(s)
What mass of magnesium does this equation show is reacting?
(Ar: Mg = 24, O = 16)
(Higher Tier Question)
24 g
48 g
12 g
16 g
In a chemical reaction involving two reactants, it is common to use one of the reactants in excess so that the other is completely used up. What do we call the reactant that is used up?
(Higher Tier Question)
Unlimited reactant
Limiting reactant
Excess reactant
Economical reactant
